Concept of excercise reaction:
The reaction between NO
and O2 is exothermic:
→ 2NO (g)
+ O2 (g) NO2 (g)
State the effects on
equilibrium
- O2 is added
- NO2 is taken out
- The temperature is increase
- The total pressure is decreased
- Neon gas is added at constant volume
- Argon gas is added at constant pressure
Answer:
1.
When
O2 gas is added
·
Equilibrium
position shift to the right in order to reduce the added O2 gas
·
As
a result, concentration of NO2 gas increase
·
Concentration
of NO and O2 gas is decrease
2.
When
NO2 is taken out
·
Equilibrium
position shift to the right in order to increase NO2 gas
·
As
a result, concentration of NO2 gas increase
·
Concentration
of NO and O2 gas is decrease
3.
The
temperature is increased
·
Equilibrium
position shift to the left in order to reduce the increase in temperature
·
As
a result, concentration of NO2 gas decrease
·
Concentration
of NO and O2 gas is increase
4. The total pressure is decreased
·
Equilibrium
position shift to the left (higher number of mole) in order to increase in
pressure
·
As
a result, concentration of NO2 gas decrease
·
Concentration
of NO and O2 gas is increase
5. Neon gas is added at constant volume
·
Partial pressure of
each reacting gas remains constant
·
Equilibbrium position
remain unchange
6. Argon gas is added at constant pressure
·
Partial pressure of
each reacting gasses decrease
·
System will respond by
increasing pressure
·
Equilibrium position
shifts to the side with higher number of moles
·
So equilibrium position
shift to the left
·
As
a result, concentration of NO2 gas decrease
·
Concentration
of NO and O2 gas is increase
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